Balance AgNO3 + Cu = Cu(NO3)2 + Ag (Silver Nitrate and Copper)

Balance AgNO3 + Cu = Cu(NO3)2 + Ag    (Silver Nitrate and Copper)

So to balance this single replacement reaction we need to write down the atoms on each side of the equation so I’ll start out with a Ag, and I have one of those Here’s the trick to balancing this equation I have an NO3 group right here And I have 2 and no 3 groups on this side so rather than split this up. I’m just gonna call it NO3, and I have one of those here and then for copper I have one copper atom on the product side for the Ag’s I have one of those for the N of threes I have 2. Two times this in parentheses that gives us 2 NO3’s 0nd then copper this to only applies to the parentheses, so I just have one copper atom So to balance equation we want to have the same number and type of atoms on each side. Silver’s those are already balanced. We have 1 No3 on the reactant side 2 on the product what I can do is put 2 in front of this AgNO3 now one of these times 2 That will equal 2 and that would balance the nitrate ion We also need to have the 2 times the 1 here so 1 times 2 that does change my silver atom so I have 2 of those and Copper have one here and one here that doesn’t change so everything’s balanced except the silvers I have two here and only one here, so I’ll just put a 2 right here, and the one time’s the 2 That’ll give me 2 and now we have balanced this equation. This is Dr. B, and thanks for watching.


  1. I know this isn't the topic being discussed but, in terms of redox, why is Copper's oxidation reduced to +2? If Copper combines with No3 (which has a charge of -1), shouldn't its oxidation number be +1 to equal CuNO3 to 0??? I need help and no videos online explaining redox seem to be able to tell me why.

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